2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO(g) + NH₂(g) → NH,NO,(s) Nitrogen NH, (9) NH, (84). HNO, (aq) HNO, (1) HNO, (9) NH.NO: (s) NH.NO: (aq) AH, (kJ/mol) AG", (kJ/mol) S (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 ΔΗ. AG AS -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the AH and AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS, was calculated in units of J/(mol"K) while AH was calculated in kl/mol. AG AG AG @ 298K @ 10K 10,000K Activate V Go to Setting
2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO(g) + NH₂(g) → NH,NO,(s) Nitrogen NH, (9) NH, (84). HNO, (aq) HNO, (1) HNO, (9) NH.NO: (s) NH.NO: (aq) AH, (kJ/mol) AG", (kJ/mol) S (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 ΔΗ. AG AS -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the AH and AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS, was calculated in units of J/(mol"K) while AH was calculated in kl/mol. AG AG AG @ 298K @ 10K 10,000K Activate V Go to Setting
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.120QP
Related questions
Question
100%
![Predict t
for the following reaction. Is entropy increasing or decreasing?
2. Calculate AH AG
and AS for the following reaction given thermodynamic data
below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values.
HNO,(g) + NH₂(g) → NH.NO,(s)
Nitrogen
NH₂ (9)
NH, (84)
HNO, (aq)
HNO, (1)
HNO.(g) + NH.) → NH.NO ST
HNO₂ (9)
NH.NO: (S)
NH.NO: (aq)
AH
AG
AS
AH, (kJ/mol) AG", (kJ/mol) S° (J/mol K)
-16.5
192.5
-27.0
111.0
-111.3
146.4
-80.7
155.6
-74.7
266.4
-183.9
151.1
-190.6
259.8
-46.1
-80.0
-207.4
-174.1
-135.1
-365.6
-339.9
3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or
nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)?
Explain.
4. Based on the signs of AH and AS, in which of the 4 categories does this reaction belong:
spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high
temperature or spontaneous at low temperature?
5. Use the A Hand AS, calculated in question 2 as well as the equation below to calculate
AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results
compare to the answers in questions 2 and 4? Be careful with the units, AS was calculated in
units of J/(mol*K) while AH was calculated in kl/mol.
AG
AG
@ 298K
@ 10K
AG @ 10,000K
Activate V
Go to Setting](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a14a4fe-84d4-4d9d-934f-c00bddb83415%2F7d1ed13f-5213-4199-bb12-cade43c001c8%2F79ilk4w_processed.png&w=3840&q=75)
Transcribed Image Text:Predict t
for the following reaction. Is entropy increasing or decreasing?
2. Calculate AH AG
and AS for the following reaction given thermodynamic data
below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values.
HNO,(g) + NH₂(g) → NH.NO,(s)
Nitrogen
NH₂ (9)
NH, (84)
HNO, (aq)
HNO, (1)
HNO.(g) + NH.) → NH.NO ST
HNO₂ (9)
NH.NO: (S)
NH.NO: (aq)
AH
AG
AS
AH, (kJ/mol) AG", (kJ/mol) S° (J/mol K)
-16.5
192.5
-27.0
111.0
-111.3
146.4
-80.7
155.6
-74.7
266.4
-183.9
151.1
-190.6
259.8
-46.1
-80.0
-207.4
-174.1
-135.1
-365.6
-339.9
3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or
nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)?
Explain.
4. Based on the signs of AH and AS, in which of the 4 categories does this reaction belong:
spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high
temperature or spontaneous at low temperature?
5. Use the A Hand AS, calculated in question 2 as well as the equation below to calculate
AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results
compare to the answers in questions 2 and 4? Be careful with the units, AS was calculated in
units of J/(mol*K) while AH was calculated in kl/mol.
AG
AG
@ 298K
@ 10K
AG @ 10,000K
Activate V
Go to Setting
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 6 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
![General Chemistry - Standalone book (MindTap Cour…](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning